In a given experiment 1.00 mole of N and 3.00 moles of H were placed in...

 

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In a given experiment 1.00 mole of N₂ and 3.00 moles of H₂ were placed in a 3.00 L container. Equilibrium was established given the following reaction: N₂(g) + 3H₂(g) + 2NH3(g) Complete the following table. Use numerical values in the Initial row and values containing the variable "x" in both the Change and Equilibrium rows. Let x = the amount of N₂ needed to reach equilibrium. Do not use spaces in expressions containing a + or - sign. K= N₂ Initial Change Equilibrium 0.333-X 0.333 Submit At equilibrium the concentration of NH3 is 0.0521 M. Determine the following quantities at equilibrium. Calculate the concentrations to 2 significant figures: [N₂] = [H₂] = M M Determine the numerical value of K for this reaction. (Enter your answer to two significant figures.) H₂ Show Hints NH3 In a given experiment 1.00 mole of N₂ and 3.00 moles of H₂ were placed in a 3.00 L container. Equilibrium was established given the following reaction: N₂(g) + 3H₂(g) + 2NH3(g) Complete the following table. Use numerical values in the Initial row and values containing the variable "x" in both the Change and Equilibrium rows. Let x = the amount of N₂ needed to reach equilibrium. Do not use spaces in expressions containing a + or - sign. K= N₂ Initial Change Equilibrium 0.333-X 0.333 Submit At equilibrium the concentration of NH3 is 0.0521 M. Determine the following quantities at equilibrium. Calculate the concentrations to 2 significant figures: [N₂] = [H₂] = M M Determine the numerical value of K for this reaction. (Enter your answer to two significant figures.) H₂ Show Hints NH3

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AnswerN2 0333 H2 33 1 M NH3 0 the change N2 x H2 3... View the full answer